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| How many elements were identified by the year 1700? What caused this rate to increase? |
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Definition
| 13; They began using scientific method to look for them |
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| Set of 3 elements w/ similar properties |
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| Who was Dmitri Mendeleev? |
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| Made the periodic table based on increasing atomic mass which allowed him to predict properties of undiscovered elements. |
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| How is todays periodic table arranged? |
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Definition
| Elements with increasing atomic number |
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| What is the periodic law? |
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Definition
| States that when elements are arranged in order of increasing atomic number, there is a periodic repitition of physical and chemical properties. |
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| What are 3 properties of metals? |
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Definition
| Ductile, Malleable, High Luster |
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| behave like metal in some conditions and non metals in other conditions. |
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| What are three things other than name, symbol, atomic number, and average atomic mass, that you can discover from a periodic table. |
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| Its electrons in each energy level, (Solid, gas, liquid) at room temp, Which group of elements it is in. |
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| What subatomic particle is key in determining the properties of an element? |
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| What are representative elements? |
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| They are group A and display a wide renge of physical & chemical properties |
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| What is atomic size? Describe how it trends on a periodic table. |
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Definition
| an atoms atomic radius then two atoms are joined together. It generally increases from top to bottom in a group bc the number of energy levels increases. Atomic size decreases left to right across a period bc electrons are added to the same energy level and are pulled closer to the nucleus by increasing numbers of protons. |
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| Ions form when atoms gain or lose electrons |
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| A positively charged cation forms when an atom loses one or more electrons -- Smaller than the atom that formed it, positive (nonmentals) |
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| A negatively charged anion forms when an atom gains one or more electrons. -- Larger than the atom that formed it, negative (metals) |
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Definition
| A measure of how much energy is required to remove an electron from an atom. |
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| Trend of Ionization Energy |
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Definition
| Decreases from top to bottom within a group and increases from left to right across a period. |
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Definition
| Metals tend to lose electrons and nonmetals tend to gain electrons. Increases from top to bottom within a group and decreases from left to right across a period. |
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| A measure of an atoms ability to attract an electron when the atom is bonded to another atom. |
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| What is the most electronegative element? |
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Definition
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| Decreases from top to bottom within a group and increases from left to right across a period. |
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| What are two variables that affect atomic sie in a group? |
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Definition
| Charge in a nucleus & Increase in occupied orbitals. |
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| Co - Transition metal - solid |
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Definition
| Ca - Alkaline earth metal - Solid |
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| Fe - Transition metal - solid |
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Definition
| Li - Alkali metal - solid |
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| Zn - Transition metal - solid |
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| Mg - Alkali metal - solid |
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| Mn - Transition metal - solid |
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| Cu - Transition metal - solid |
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| Cr - Transition metal - solid |
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| Ni - Transition metal - solid |
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| Cd - Transition metal - solid |
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| Hg - Transition metal - liquid |
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Definition
| It has to do with how easily electrons come off of an atom which then deals with atom size |
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| Co - Transition metal - solid |
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| Ca - Alkaline earth metal - Solid |
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| Fe - Transition metal - solid |
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| Li - Alkali metal - solid |
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| Zn - Transition metal - solid |
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| Mg - Alkali metal - solid |
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| Mn - Transition metal - solid |
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| Cu - Transition metal - solid |
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| Cr - Transition metal - solid |
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| Ni - Transition metal - solid |
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| Cd - Transition metal - solid |
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| Hg - Transition metal - liquid |
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| It has to do with how easily electrons come off of an atom which then deals with atom size |
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